The suggested mechanism of a reaction is :
(a) `A+BhArrD("fast) " (b)A+Drarr2C("slow")`
Write the balanced equation of the reaction if its experimentally deduced rate equation is , rate `k=[A]^(2)[B]` Find the intermediate formed during the course of the reaction . Does the predicted rate law from the mechanism match the experimental rate law ?

Explanation

The overall reaction is the sum of the reaction (a) and (b) i.e., `2A+Brarr2C`
Here the intermediate is D.
Now , `A+BhArrD,`
`k=([D])/([A][B]) ("K = rate constant")" "...[1]`
Rate equation of the slowest step
`k=[A][D]=k[A]xxK[A][B]`
`=kK[A]^(2)[B]=k'[A]^(2)[B]` (where , kK=k')
Yes , the predicted rate law from the mechanism matches the experimental rate law.